Ionic equations and solubility rules

what are the steps for writing ionic equations?

1. write the full balanced equation with state symbols

2. separate aqueous, ionic compounds into ions

3. remove spectator ions

silver ion formula

Ag⁺

ammonium formula

NH_4⁺

copper ion formula

Cu²⁺

zinc ion formula

Zn²⁺

hydroxide ion formula

OH^-

nitrite ion formula

NO_2^-

nitrate ion formula

NO_3^-

hydrogencarbonate ion formula

HCO_3^-

sulphate ion formula

SO_4^2-

carbonate ion formula

CO_3^2-

phosphate ion formula

PO_4^3-

soluble salts:

• all nitrates

• sodium, potassium, ammonium

• most common chlorides

• most common sulfates

• sodium, potassium, ammonium carbonates

• sodium, potassium, ammonium hydroxides

sparingly soluble salts:

• silver, calcium sulfates

• barium, calcium hydroxides

insoluble salts:

• lead (ii), silver chloride

• lead (ii), barium sulfate

• most common carbonates

• most common hydroxides

what elements are diatomic?

group 7 and: H2, N2, O2

acid + metal —>

salt + hydrogen

acid + hydroxide —>

salt + water

acid + oxide —>

salt + water

acid + carbonate —>

salt + water + carbon dioxide

why are some ions considered spectator ions?

• they are unchanged in state, formula and charge

why are ionic equations used?

they only show the species that undergo chemical change, simplifying the reaction to the essential process.